Preview Lesson Starter Objectives Accuracy and Precision Significant Figures Scientific Notation Using Sample Problems Direct Proportions Inverse Proportions Chapter 2 Section 3 Using Scientific Measurements

Lesson Starter Look at the specifications for electronic balances. How do the instruments vary in precision? Discuss using a beaker to measure volume versus using a graduated cylinder. Which is more precise? Section 3 Using Scientific Measurements Chapter 2

Objectives Distinguish between accuracy and precision. Determine the number of significant figures in measurements. Perform mathematical operations involving significant figures. Convert measurements into scientific notation. Distinguish between inversely and directly proportional relationships. Section 3 Using Scientific Measurements Chapter 2

Accuracy and Precision Accuracy refers to the closeness of measurements to the correct or accepted value of the quantity measured. Precision refers to the closeness of a set of measurements of the same quantity made in the same way. Section 3 Using Scientific Measurements Chapter 2

Accuracy and Precision Section 3 Using Scientific Measurements Chapter 2

Click below to watch the Visual Concept. Visual Concept Chapter 2 Section 3 Using Scientific Measurements Accuracy and Precision

Accuracy and Precision, continued Percentage Error Percentage error is calculated by subtracting the accepted value from the experimental value, dividing the difference by the accepted value, and then multiplying by 100. Section 3 Using Scientific Measurements Chapter 2

Accuracy and Precision, continued Sample Problem C A student measures the mass and volume of a substance and calculates its density as 1.40 g/mL. The correct, or accepted, value of the density is 1.30 g/mL. What is the percentage error of the student’s measurement? Section 3 Using Scientific Measurements Chapter 2

Accuracy and Precision, continued Sample Problem C Solution Section 3 Using Scientific Measurements Chapter 2

Accuracy and Precision, continued Error in Measurement Some error or uncertainty always exists in any measurement. skill of the measurer conditions of measurement measuring instruments Section 3 Using Scientific Measurements Chapter 2

Significant Figures Significant figures in a measurement consist of all the digits known with certainty plus one final digit, which is somewhat uncertain or is estimated. The term significant does not mean certain. Section 3 Using Scientific Measurements Chapter 2

Reporting Measurements Using Significant Figures Section 3 Using Scientific Measurements Chapter 2

Significant Figures, continued Determining the Number of Significant Figures Section 3 Using Scientific Measurements Chapter 2

Click below to watch the Visual Concept. Visual Concept Chapter 2 Section 3 Using Scientific Measurements Rules for Determining Significant Zeros

Significant Figures, continued Sample Problem D How many significant figures are in each of the following measurements? a g b cm c. 910 m d L e kg Section 3 Using Scientific Measurements Chapter 2

Sample Problem D Solution a.28.6 g There are no zeros, so all three digits are significant. b cm By rule 4, the zero is significant because it is immediately followed by a decimal point; there are 4 significant figures. c. 910 m By rule 4, the zero is not significant; there are 2 significant figures. Section 3 Using Scientific Measurements Chapter 2 Significant Figures, continued

Sample Problem D Solution, continued d L By rule 2, the first two zeros are not significant; by rule 1, the third zero is significant; there are 4 significant figures. e kg By rule 2, the first three zeros are not significant; by rule 3, the last three zeros are significant; there are 5 significant figures. Section 3 Using Scientific Measurements Chapter 2 Significant Figures, continued

Rounding Section 3 Using Scientific Measurements Chapter 2

Click below to watch the Visual Concept. Visual Concept Chapter 2 Section 3 Using Scientific Measurements Rules for Rounding Numbers

Significant Figures, continued Addition or Subtraction with Significant Figures When adding or subtracting decimals, the answer must have the same number of digits to the right of the decimal point as there are in the measurement having the fewest digits to the right of the decimal point. Addition or Subtraction with Significant Figures For multiplication or division, the answer can have no more significant figures than are in the measurement with the fewest number of significant figures. Section 3 Using Scientific Measurements Chapter 2

Sample Problem E Carry out the following calculations. Express each answer to the correct number of significant figures. a m m b. 2.4 g/mL  mL Section 3 Using Scientific Measurements Chapter 2 Significant Figures, continued

Sample Problem E Solution a.5.44 m m = 2.84 m Section 3 Using Scientific Measurements Chapter 2 Significant Figures, continued There should be two digits to the right of the decimal point, to match 5.44 m. b. 2.4 g/mL  mL = 38 g There should be two significant figures in the answer, to match 2.4 g/mL.

Significant Figures, continued Conversion Factors and Significant Figures There is no uncertainty exact conversion factors. Most exact conversion factors are defined quantities. Section 3 Using Scientific Measurements Chapter 2

In scientific notation, numbers are written in the form M × 10 n, where the factor M is a number greater than or equal to 1 but less than 10 and n is a whole number. example: mm = 1.2 × 10 −4 mm Scientific Notation Section 3 Using Scientific Measurements Chapter 2 Move the decimal point four places to the right and multiply the number by 10 −4.

Scientific Notation, continued 1. Determine M by moving the decimal point in the original number to the left or the right so that only one nonzero digit remains to the left of the decimal point. 2. Determine n by counting the number of places that you moved the decimal point. If you moved it to the left, n is positive. If you moved it to the right, n is negative. Section 3 Using Scientific Measurements Chapter 2

Scientific Notation, continued Mathematical Operations Using Scientific Notation 1. Addition and subtraction —These operations can be performed only if the values have the same exponent (n factor). example: 4.2 × 10 4 kg × 10 3 kg or Section 3 Using Scientific Measurements Chapter 2

2. Multiplication —The M factors are multiplied, and the exponents are added algebraically. example: (5.23 × 10 6 µm)(7.1 × 10 −2 µm) = (5.23 × 7.1)(10 6 × 10 −2 ) = × 10 4 µm 2 = 3.7 × 10 5 µm 2 Section 3 Using Scientific Measurements Chapter 2 Scientific Notation, continued Mathematical Operations Using Scientific Notation

3. Division — The M factors are divided, and the exponent of the denominator is subtracted from that of the numerator. example: Section 3 Using Scientific Measurements Chapter 2 Scientific Notation, continued Mathematical Operations Using Scientific Notation = × 10 3 = 6.7  10 2 g/mol

Click below to watch the Visual Concept. Visual Concept Chapter 2 Section 3 Using Scientific Measurements Scientific Notation

Using Sample Problems Analyze The first step in solving a quantitative word problem is to read the problem carefully at least twice and to analyze the information in it. Plan The second step is to develop a plan for solving the problem. Compute The third step involves substituting the data and necessary conversion factors into the plan you have developed. Section 3 Using Scientific Measurements Chapter 2

Using Sample Problems, continued Evaluate Examine your answer to determine whether it is reasonable. 1. Check to see that the units are correct. 2. Make an estimate of the expected answer. 3. Check the order of magnitude in your answer. 4. Be sure that the answer given for any problem is expressed using the correct number of significant figures. Section 3 Using Scientific Measurements Chapter 2

Using Sample Problems, continued Sample Problem F Calculate the volume of a sample of aluminum that has a mass of kg. The density of aluminum is 2.70 g/cm3. Section 3 Using Scientific Measurements Chapter 2

Using Sample Problems, continued Sample Problem F Solution 1.Analyze Given: mass = kg, density = 2.70 g/cm3 Unknown: volume of aluminum 2.Plan The density unit is g/cm3, and the mass unit is kg. conversion factor: 1000 g = 1 kg Rearrange the density equation to solve for volume. Section 3 Using Scientific Measurements Chapter 2

Using Sample Problems, continued Sample Problem F Solution, continued 3. Compute Section 3 Using Scientific Measurements Chapter 2 = cm 3 (calculator answer) round answer to three significant figures V = 1.13 × 10 3 cm 3

Using Sample Problems, continued Sample Problem F Solution, continued 4. Evaluate Answer: V = 1.13 × 10 3 cm 3 The unit of volume, cm 3, is correct. An order-of-magnitude estimate would put the answer at over 1000 cm 3. Section 3 Using Scientific Measurements Chapter 2 The correct number of significant figures is three, which matches that in 2.70 g/cm.

Direct Proportions Two quantities are directly proportional to each other if dividing one by the other gives a constant value. read as “y is proportional to x.” Section 3 Using Scientific Measurements Chapter 2

Direct Proportion Section 3 Using Scientific Measurements Chapter 2

Inverse Proportions Two quantities are inversely proportional to each other if their product is constant. read as “y is proportional to 1 divided by x.” Section 3 Using Scientific Measurements Chapter 2

Inverse Proportion Section 3 Using Scientific Measurements Chapter 2

Click below to watch the Visual Concept. Visual Concept Chapter 2 Section 3 Using Scientific Measurements Direct and Inverse Proportions